SYBSc Chemistry sem III IV_1 Syllabus Mumbai University by munotes
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AC – 27/06/2023
Item No. 6.1 (R)
UNIVERSITY OF MUMBAI
Revised Syllabus for
S.Y. B.Sc.
(Chemistry)
Semester: III & IV
(CBCS)
(With effect from the academic year 2023 -24)
Page 4
Page 5
UNIVERSITY OF MUMBAI
Essentials Element s of The Syllabus
1 Title of Course Syllabus for two semester S. Y. B. Sc.
course in chemistry
2 Course Code USCH301, USCH302, USCH303
USCH401, USCH402, USCH404
USCHP1 to USCHP6
3 Preamble Attached
4 Objective To infuse in the learner a spirit of
inquiry into the fundamental aspects
of the various core areas of
Chemistry.
To make the learner proficient in
analyzing the various observations
and chemical phenomena presented
to him during the course.
To make the learner capable of
solving problems in the various
units of this course
To give the learner an opportunity
to get hands on experience of the
various concepts and processes in
the various branches of chemistry
To impart various skills of handling
chemicals, reagents, apparatus,
instruments and the care and safety
aspects involved in such handling
To make the learner capable of
analysing and interpreting results of
the experiments he conducts or
performs
5 Eligibility Pass F. Y. B. Sc.
6 Fee Structure As Per Guidelines issued from the
University
7 No. of Lectures 9 lectures per week (three lectures per
paper)
Page 6
8 No. of Practicals 9 periods per week (three periods per
paper)
9 Duration of Course Two Semester
10 Notional Hours 72 hours per paper per semester Theory
and 36 hours per paper per semes ter for
laboratory sessions
11 No of students per batch 120 students per division (20 Students for
laboratory sessions)
12 Selection As per merit.
13 Assessment End of semester examination of 75
marks per paper for theory , 25 marks
Internal evaluation and 50
marks per paper for laboratory sessions
14 Syllabus Detail Attached
15 Title of the Unit As given in the Syllabus text
16 Title of the Sub-unit As given in the syllabus text.
17 Semester wise Theory As prescribed in the syllabus text
18 Semester wise Practicals As prescribed in the syllabus text.
19 Question Paper Pattern As prescribed by the Faculty of Science
20 Scheme of evaluation of
Project N.A.
21 List of suggested reading --
22 List of websites --
23 List of You Tube videos --
24 List of MOOCs --
Page 7
REGULATIONS
1. Preamble and objectives of the Course :
In the first two semesters of the six semester graduation program of
B. Sc.(Chemistry) the learner was introduced to some basic aspects in the
various core branches of chemistry like Physi cal Chemistry, Organic
chemistry and Inorganic chemistry. Concepts about the structure of atom,
distribution of electrons, Thermodynamics, Formation of organic
compounds and basic ideas in reactivity of molecules in general and
organic compounds in particu lar were introduced to the learner. He was
made inquisitive about why and how should atoms combine to give
molecules or ions. The non -orbital approach to appreciating the shapes of
polyatomic species in general and molecules in particular.
The story of che mistry is taken further in the coming two semesters
of the second year of the B. Sc. (Chemistry) Program. However it is also
realised that some students opting for the course on Chemistry may not
continue with the subject subsequently as such the syllabus is designed to
retain the interest of the serious learner of chemistry as well as be helpful
to non -chemistry learners. With such students who would want to pursue
other branches of science but would want to acquire a basic appreciation
and experience of c hemistry a separate paper (Paper -III) is designed. This
paper along with the laboratory session unit that goes with it deals with the
basics of chemical analysis, separating components from a given sample,
basic concepts like pH, experimental techniques li ke Titrimetry,
Gravimetry, using instruments to carry out analysis, the various techniques
like chromatography, electrophoresis, Instrumentation in general is felt to
be of interest to learners of various branches like physics, botany, zoology,
and microbi ology.
The major objectives of B.Sc. Chemistry course are
To infuse in the learner a spirit of inquiry into the fundamental aspects
of the various core areas of Chemistry.
Page 8
To make the learner proficient in analysing the various observations and
chemical p henomena presented to him during the course.
To make the learner capable of solving problems in the various units of
this course
To give the learner an opportunity to get hands on experience of the
various concepts and processes in the various branches of chemistry
To impart various skills of handling chemicals, reagents, apparatus,
instruments and the care and safety aspects involved in such handling
To make the learner capable of analyzing and interpreting results of the
experiments he conducts or perform s
To make the learner capable of acquiring or pursuing a source of
livelihood like jobs in chemical industry
To arouse the interest to pursue higher levels of learning in chemistry,
2. Condition for Admission
A candidate who has passed the F.Y.B.Sc. of Mumba i University or
an examination of some other university accepted by the syndicate as
equivalent there to with Chemistry, Physics, Maths, Botany, Zoology or
Life Science shall be eligible for admission into S.Y.B.Sc., course in
Chemistry.
3. Duration of the Course: one year
4. Course of study:
Page 9
Draft copy of the proposed revised syllabus for
Choice Based Credit System
S.Y.B.Sc. Chemistry
To be implemented from the Academic year 2023-2024
For the subject of chemistry there shall be three papers for 45 lectures each comprising of
three units of 15 L each.
Semester -III
1. Paper -I (General Chemistry) Unit-I Physical Chemistry
Unit-II Inorganic Chemistry
Unit-III Organic Chemistry.
2. Paper -II (General Chemistry) Unit-I Physical Chemistry
Unit-II Inorganic Chemistry
Unit-III Organic Chemistry.
3. Paper III (Basics of Analytical Chemistry )
Semester -IV
1. Paper -I (General Chemistry) Unit-I Physical Chemistry
Unit-II Inorganic Chemistry
Unit-III Organic Chemistry.
2. Paper -II (General Chemistry) Unit-I Physical Chemistry
Unit-II Inorganic Chemistry
Unit-III Organic Chemistry.
3. Paper III (Basics of Analytical Chemistry)
Page 10
Choice Based Credit System
S. Y. B. Sc.
Chemistry Syllabus
To be implemented from the Academic year 2023-2024
Course Content
Semester III
Course
Code Unit Topics Credits L/Week
USCH301 I Chemical Thermodynamics -II,
Electrochemistry
2 1
II
Chemical Bonding 1
III Reactions and reactivity of halogenated
hydrocarbons, alcohols, phenols and epoxides 1
USCH302 I Chemical Kinetics -II, Solutions , Polymer
Chemistry -I 2 1
II Selected topics on p block elements 1
III Carbonyl Compounds 1
USCH303 I Introduction to Analytical Chemistry and Statistical
Treatment of analytical data-I
2 1
II Classical Methods of Analysis. 1
III Instrumental Methods -I 1
USCHP1 Chemistry Practicals I 1 3
USCHP2 Chemistry Practicals II 1 3
USCHP3 Chemistry Practicals III 1 3
Semester IV
Course
Code Unit Topics Credits L/Week
USCH401 I Electrochemistry -II, Phase Equilibria
2 1
II Comparative Chemistry of the transition metals &
Coordination Chemistry 1
III Carboxylic acids and their derivatives, Sulphonic
acids 1
USCH402 I Solid state, Catalysis
2 1
II Ions in aqueous medium & Uses and Environmental
Chemistry of Volatile Oxides and oxo -acids 1
III Amines, Diazonium salts, Heterocyclic compounds 1
USCH403 I Methods of separation
2 1
II Instrumental Methods -II 1
III Statistical Treatment of analytical data --II 1
USCHP4 Chemistry Practicals I 1 3
USCHP5 Chemistry Practicals II 1 3
USCHP6 Chemistry Practicals III 1 3
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Semester III
Paper I
Theory: 45 Lectures
Unit I: Physical Chemistry
1.1 Chemical Thermodynamics -II(8L)
1.1.1 Free Energy Functions: Helmholtz Free Energy, Gibb's Free Energy, Variation of Gibb's
free energy with Pressure and Temperature.
1.1.2 Gibbs -Helmholtz equation, van't Hoff reaction isotherm and van't Hoff reaction
isochore.
(Numericals expected).
1.1.3 Thermodynamics of Open System: Partial Molal Properties, Chemical Potential and its
variation with Pressure and Temperature, Gibb's Duhem equation.
1.1.4 Concep t to fugacity and Activity .
1.2 Electrochemistry: (7L)
1.2.1 Electrolytes: Definition, Strong and Weak electrolytes and their conductance measurement ,
ions and electrical conductivity by ions.
1.2..2 Kohlrausch law of independ ent migration of ions.
1.2.3 Applications of conductance measurements: determination of degree of ionization and
ionization constant of weak electrolyte, solubility and solubility product of sparingly soluble
salts, ionic product of water . (Numerical expe cted).
1.2.4 Transference number and its experimental determination using Moving boundary method .
(Numericals expected).Factors affecting transference number.
Unit-II: Inorganic Chemistry
2. Chemical Bonding
2.1 Non-Directional Bonding (4L)
2.1.1 Ionic Bond: Cond itions for the Formation of Ionic Bond.
2.1.2 Types of Ionic Crystals
2.1.3 Radius Ratio Rules
2.1.4 Born -Haber Cycle and its Application
2.2. Directional Bonding: Orbital Approach. (6L)
2.2.1 Covalent Bonding , The Valence Bond Theory - Introduction and basic tenets.
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2.2.2 Interaction betw een two hydrogen atoms and the Potential energy diagram of the resultant
system.
2.2.3 Corrections applied to the system of two hydrogen atoms -Formation of H2
2.2.4 Definition , concept of Homonuclear diatomic molecules only for He2 & Ne2 molecules.
2.2.5 Resonance and the Concept of Formal Charge; Rules for Resonance or Canonical Structures .
2.2.6 Bonding in Polyatomic Species: The Role of Hybridization. And types of hybrid orbitals -
sp,sp2,sp3, sp3d, sp2d2andsp2d sp3d2.
2.2.7 Equivalent and Non-Equivalent hybrid orbitals
2.3 Molecular Orbi tal Theory (5L)
2.3.1. Comparing Atomic Orbitals and Molecular Orbitals.
2.3.2. Linear combination of atomic orbitals to give molecular orbit als LCAO -MO approach for
diatomic homonuclear molecules).
2.3.3 Molecular orbital Theory and Bond Order and magnetic property: w ith reference toO 2,O2+O2-,O22-
(Problemsandnumericalproblemsexpectedwhereverpossible)
Unit III: Organic Chemistry
3.1. Reactions and reactivity of halogenated hydrocarbons: [4L]
3.1.1.Alkyl halides: Nucleophilic substitution reactions: SN1, SN2 and SNi m echanisms with
stereochemical aspects and factors affecting nucleophilic substitution reactions , nature of substrate,
solvent, nucleophilic reagent and leaving group.
3.1.1. Aryl halides: Reactivity of aryl halides towards nucleophilic substitution reacti ons. Nucleophilic
aromatic substitution (SNAr) addition -elimination mechanism and benzyne mechanism.
3.1.2.Organomagnesium and organolithium compounds: [3L]
Nomenclature, nature, type and reactivity of carbon -metal bond. Preparation using alkyl / aryl hal ide.
Structure, stability and reactions with compounds containing acidic hydrogen, carbonyl compounds,
CO 2, cyanides and epoxides.
3.2 Alcohols, phenols and epoxides: [8L]
3.2.1. Alcohols: Nomenclature, Preparation: Hydration of alkenes, hydrolysis of a lkyl halides, reduction of
aldehydes and ketones, using Grignard reagent. Properties: Hydrogen bonding, types and effect of
hydrogen bonding on different properties. Acidity of alcohols, Reactions of alcohols
3.2.2.Phenols: Preparation, physical propertie s and acidic character. Comparative acidic strengths of
alcohols and phenols, resonance stabilization of phenoxide ion. Reactions of phenols.
3.2.3.Epoxides: Nomenclature, methods of preparation and reactions of epoxides: reactivity, ring-opening
reaction s by nucleophiles (a) In acidic conditions: hydrolysis, reaction with halogen halide, alcohol,
hydrogen cyanide. (b) In neutral or basic conditions: ammonia, amines, Grignard reagents, alkoxides
Page 13
Semester III
Paper II
Unit I: Physical Chemistry
1.1 Chemical Kinetics -II (5L)
1.1.1 Introduction to reaction mechanism (concept of elementary steps, intermediates, and the overall
reaction mechanism with an example of Thermal chain reactions: H 2. and Br 2. reaction.
1.1.2 Types of Complex Chemical reactions: Reversible or opposing, consecutive and parallel
reactions
(No derivations, only examples expected ),
1.2 Solutions: (6 L)
1.2.1 Thermodynamics of ideal solutions: Ideal solutions and Raoult’s law, deviations from Ra oult’s
law–non-ideal solutions. Vapo ur pressure -composition and temperature -composition curves of
ideal and non -ideal solutions. Azeotropes and Zeotropes definition and significance in solution
behavior
1.2.2 Partial miscibility of liquids: Definition, Effect of Temperature, effect of impur ity and
intermolecular interactions on partial miscibility, Critical solution temperature;
Phenol -Water, Triethanolamine – Water and Nicotine – Water systems
1.2.3 Immiscibility of liquids - Nernst distribution law and its applications, solvent extraction. .
1.3 Polymer Chemistry – I (4L)
1.3.1 Basic Terms: Macromolecule, monomer, repeat unit, Polymerisation, (addition and condensation
polymerization ) Degree of Polymerisation
1.3.2 Polymer structures linear, branched and cross -linked
1.3.3 Molecular weight of Polym ers: Definition and formulae of Number average molecular weight,
weight aver age molecular weight Z- average molecular weight, and viscosity average molecular
weight.
(numerical expected)
Unit -II: Inorganic Chemistry
2. Selected topics on p -block ele ments (15L)
2.1 Chemistry of Boron Compounds
2.1.1 Electron deficient compounds –BH 3,BF 3,BCl 3with respect to Lewis acidity and applications.
2.1.2 Preparation of simple boranes like diborane and tetraborane.
2.1.3 Structure and bonding in diborane and tetraborane(2e -3cbonds)
2.1.4 Synthesis of Borax.
2.2 Chemistry of Silicon
2.2.1 Silicon compounds : Occurrence, Structure and Inertness of SiO 2
2.2.2 Preparation of structure of SiCl 4
2.2.3 Preparation of extra -pure Silicon
2.3 Chemistry of Nitrogen family
2.3.1 Trends in chemical reactivity - Formation of hydrides, halides, oxides with special reference
to oxides of nitrogen.
2.3.2 Oxides of nitrogen with respect to preparation and structure of NO, NO 2,N2O and N2O4.
Page 14
Unit III: Organic Chemistry
3. Carbonyl Compounds: [15L]
3.1 Nomenclature of aliphatic, alicyclic and ar omatic carbonyl compounds. Structure, reactivity of
aldehydes and ketones and methods of preparation; Oxidation of primary and secondary alcohols
using PCC, hydration of alkynes, Rosenmund reduction and Gattermann – Koch formylation
3.2 General mechanism of nucleophilic addition, and acid-catalyzed nucleophilic addition reactions.
3.3 Reactions of aldehydes and ketones with NaHSO 3, HCN, RMgX, alcohol, amine, phenylhydrazine ,
2,4-Dinitrophenyl hydrazine, LiAlH 4 and NaBH 4.
3.4 Mechanisms of following reactio ns: Benzoin condensation, Knoevenagel condensation, Claisen -
Schmidt and Cannizzaro reaction.
3.5 Keto -enol tautomerism: Mechanism of acid and base catalyzed enolization
3.6 Active methylene compounds: Acetylacetone, ethyl acetoacetate diethyl malonate, stabilized enols.
Alkylation of Acetylacetone and ethyl acetoacetate
Page 15
Semester IV
Paper I
Theory: 45 Lectures
Unit I: Physical Chemistry
1.1Electrochemistry -II: (8 L)
1.1.1 Electrochemical cells, Nernst equation and its importance in generating electricity through chemical
reactions. Types of electrochemical cells - Reversible and irreversible cells (Definition, example,
characteristics)
1.1.2 Types of electrodes, Standard electrode potential, Electrochemical series.
1.1.3 Thermodynamics of a reversible cell, calculation of thermodynamic properties: ΔG, ΔH and ΔS from
EMF data.
1.1.4 Calculation of equilibrium constant and pH measurement using Hydrogen electrode and quinhydrone
electrode, from EMF data.
1.1.5 Applicat ion of electrochemistry in the field of –‘Hydrogen Clean energy ’ and the role of Batteries in
clean energy storage.
(Numericals to be solved wherever necessary)
1.2 Phase Equilibria: (7L)
1.2.1 Introduction to Phase equilibria, Phases, components and de grees of freedom of a system, criteria of
phase equilibrium. Gibbs Phase Rule.
1.2.2 Derivation of Clausius – Clapeyron equation and its importance in phase equilibria.
1.2.3 Phase diagrams of one -component systems (water and sulphur).
1.2.4 Two-component systems involving eutectics – Condensed Phase rule, Definition of eutectic Phase
diagram of Lead -Silver system.
1.2.5 Application of Phase equilibria in
ii). Industry – metallurgy
iii). Energy and environmental engineering
iiii). Food and beverage industry
iiv). Pharmaceutical in dustry .
Unit -II: Inorganic Chemistry
2.1 Comparative Chemistry of the transition metals (9L)
2.1.1 Position in the periodic table; Natural occurrence principal ores and minerals ;
2.1.2 Significance of special stability of d0, d5 and d10 leading to variabl e oxidation states; Unusual
oxidation states and their stabilities in aqueous solutions (with special reference to vanadium,
and chromium.)
2.1.3 Origin of color for transition metals and their compounds: such as reflectivity , surface coatings,
particle si ze, packing density for metals and nature of d-orbitals, number of electrons in the d -
orbitals, geometry, and ability for charge transfer).
2.1.4 Magnetic properties of transition metal compounds: Origin of magnetism -spin and orbital
motion of electrons; equation for spin only and spin -orbital magnetism in terms of Bohr
magnetons (No derivation of relevant equations expected); Reasons for quenching of orbital
moments.
Page 16
2.1.5 Qualitative tests for transition metal ions: General considerations indevising tests (with
reference to Chromium, Manganese, Iron, Cobalt Nickel and Copper)
2.2 Coordination Chemistry: (6L)
2.2.1 Introduction to Chemistry of Coordination Compounds
i. Historical perspectives : Early ideas on coordination compounds
ii. Basic terms and nomenclature.
iii. Types of ligands
iv. Isomerism: General Types with special reference to stereo isomerism of coordination
compounds (C.N=6)
v. Evidence for the formation of coordination compounds.
2.2.2 Theories of coordination compounds
i. Werner’s Theor y of coordination compounds,
ii. Effective atomic number rule.
iii. Eighteen electron Rule
2.2.3 Nature of the Metal -Ligand Bond:
i. Valence Bond Theory; Hybridisation of the central metal orbitals -sp3d2/d2sp3
ii. Inner and outer orbital complexes of .(sui table examples of Mn(II)Fe(II), Fe(III),
Co(II)/Co(III), Ni(II), Cu(II) Zn(II) complexes with ligands like aqua, ammonia CN-and
halides may be used)
iii. Limitations of V.B.T
2.2.4 Application of coordination compounds .
Unit III: Organic Chemistry
3.1 C arboxylic Acids and their Derivatives :(11 L)
3.1.1. Nomenclature, structure and physical properties, acidity of carboxylic acids, effects of substituents on
acid strength of aliphatic and aromatic carboxylic acids.
3.1.2. Preparation of carboxylic acid s: oxidation of alcohols and alkyl benzene, carbonation of Grignard and
hydrolysis of nitriles.
3.1.3. Reactions: Acidity, salt formation, decarboxylation, Reduction of carboxylic acids with LiAlH 4,
diborane, Hell -Volhard -Zelinsky reaction, Conversion of carboxylic acid to acid chlorides, esters,
amides and acid anhydrides and their relative reactivity.
3.1.4. Mechanism of nucleophilic acyl substitution and acid-catalyzed nucleophilic acyl substitution.
Interconversion of acid derivatives by nucleophili c acyl substitution.
3.1.5. Mechanism of Claisen condensation and Dieckmann condensation
3.2 Sulphonic acids: [4L]
Nomenclature, preparation of aromatic sulphonic acids by sulphonation of benzene (with mechanism), toluene
and naphthalene, Reactions: Acidi ty of arene sulfonic acid, Comparative acidity of carboxylic acid and sulfonic
acids. Salt formation, desulphonation. Reaction with alcohol, phosphorous pentachloride, IPSO substitution
Page 17
Semester IV
Paper II
Unit I: Physical Chemistry
Solid State: (7L)
1.1.1 laws of Crystallography and Types of Crystals
1.1.2 Characteristics of simple cubic, face-centered cubic and body -centered cubic systems, interplanar
distance in a cubic lattice (only expression for ratio of interplanar distances are expected)
1.1.3 Use of X-rays in the study of crystal structure, Bragg’s equation (derivation expected ), X-rays diffraction
method of studying crystal lattice structure , structure of NaCl and KCl. Determination of Avogadro’s
number (Numericals expected)
Catalysis: (8 L)
1.2.1 Types of catalysis, catalytic activity, specificity and selectivity, inhibitors, catalyst poisoning and
deactivation
1.2.2 Mechanisms and kinetics of acid-base catalyzed reactions, effect of pH.
1.2.3 Mechanisms and kinetics of enzyme catalyzed reactions (Michaelis -Menten equation)
1.2.4 Nanoparticles as catalyst – basic concepts, their importance in chemical reactions, properties and their
application in energy conversion(fuel cells and solar cells) Challenges associated with nanoparticles as
catalyst.
Unit -II: Inorganic Chemistry
2. Ions in aqueous medium
2.1 Acidity of Cations and Basicity of Anions (8L)
i. Hydration of Cations; Hydrolysis of Cations predicting degree of hydrolysis of Cations -effect of
Charge and Radius .
ii. Classification of ca tions on the basis of acidity category – Non-acidic , Moderately acidic,
strongly acidic, very strongly acidic with pKa values range and examples
iii. Hydration of Anions; Effect of Charge and Radius; Hydration of anions -concept, diagram
classification on the basis of basicity
2.2 Uses and Environmental Chemistry of volatile Oxides and oxo-acids (7L)
i. Physical properties of concentrated oxo -acids like sulfuric, Nitric and Phosphoric acid
ii. Uses and environmental aspects of these acids.
Unit III: Organic Chemistry
3.1Nitrogen containing compounds (7L)
3.1.1 Amines:(4L)
Nomenclature, effect of substituent on basicity of aliphatic and aromatic amines Preparation: Reduction of
aromatic nitro compounds using catalytic hydrogenation, chemical reduction using Fe-HCI, Sn -HCl, Zn -acetic
acid, reduction of nitriles, ammonolysis of halides, reductive amination, Hoffmann bromamide reaction
Reactions - Salt Formation, N -acylation, N -alkylation, Hofmann’s exhaustive methylation (HEM), Hofmann -
elimination reaction, reac tion with nitrous acid, carbylamine reaction, Electrophilic substitution in aromatic
amines: bromination, nitration and sulphonation
Page 18
3.1.2 Diazonium Salts:(3L)
Preparation and their reactions/synthetic application - Sandmeyer reaction, Gattermann reaction , Gomberg
reaction, Replacement of diazo group by -H,-OH. Azo coupling with phenols, naphthols and aromatic amines,
reduction of diazonium salt to aryl hydrazine and hydroazobenzene
3.2 Heterocyclic Compounds: (8L)
3.2.1. Classification, nomenclature of 5- and 6 -membered rings containing one heteroatom
3.2.2. Synthesis of Furan, Pyrrole (Paal -Knorr synthesis, Knorr pyrrole synthesis, and Hantzsch
synthesis), Thiophene, Pyridine (Hantzsch synthesis)
3.2.3. Reactivity of furan, pyrrole and thiophene toward s electrophilic substitution reactions on the basis
of stability of intermediate and of pyridine on the basis of electron distribution. Reactivity of
pyridine towards nucleophilic substitution on the basis of electron distribution.
3.2.4. Reactions of fur an, pyrrole and thiophene: halogenation, nitration, sulphonation, Vilsmeier -Haack
reaction, Friedel -Crafts reaction. Furan: Diels -Alder reaction, Ring opening. Pyrrole: Acidity and
basicity of pyrrole. Comparison of basicity of pyrrole and pyrrolidine.
3.2.5. Pyridine: Basicity. Comparison of basicity of pyridine, pyrrole and piperidine. Sulphonation of
pyridine (with and without catalyst), reduction and action of sodamide (Chichibabin reaction)
Page 19
Semester III
Chemistry Practicals:
Unit I: Physical Chemis try
1. To verify Ostwald’s dilution law for weak acid conductometrically.
2. To determine dissociation constant of weak acid conductometrically.
3. To determine the critical solution temperature (CST) of phenol - Water System.
4. Determination of energy of activation of acid-catalyzed hydrolysis of methyl acetate.
5. To investigate the reaction between K2S2O8 and KI with equal initial concentrations of
the reactants
6. To determine solubility of sparingly soluble salts (any two) conductometrically.
Unit II: Inorganic Chemi stry
1. Identification of cations in a given mixture and Analytically separating them
[From a mixture containing not more than two of the following: Pb(II), Ba(II), Ca(II),
Sr (II), Cu(II), Cd(II), Mg(II), Zn(II), Fe(II), Fe(III), Ni(II), Co(II) Al(III), Cr( III)]
2. Crystallisation of potassium iodate and to estimate its purity before and after the
separation.
3. Estimation of total hardness
4. Investigation of the raction between Copper supfate and Sodium Hydroxide
(Standard EDTA solution to be provided to the learne r).
Unit III: Organic Chemistry
Short organic preparation and their purification: Use 0.5-1.0g of the organic compound.
Purify the product by recrystallization. Report theoretical yield, percentage yield and
melting point of the purified product.
Prepara tion of:
1. Cyclohexanone oxime from cyclohexanone.
2. Glucosazone from dextrose or fructose
3. Tribromoaniline from aniline.
4. β-Naphthylbenzoate
5. m-Dinitrobenzene from nitrobenzene
6. Phthalic anhydride from phthalic acid by sublimation
7. Acetanilide from aniline
8. p-Brom oacetanilide from acetanilide
9. Iodoform from acetone
(Any eight preparations)
Page 20
Semester IV
Chemistry Practicals:
Unit I: Physical Chemistry
1. To determine standard EMF and the standard free energy change of Daniel cell
potentiometrically.
2. To determine the amount of HCl in the given sample potentiometrically.
3. Compare the strengths of HCl and H 2SO 4 by studying kinetics of acid hydrolysis of
methyl acetate.
6. Industrial visit report.
Unit II: Inorganic Chemistry
1. Inorganic preparation – Nickel dimethyl glyoxime using microscale method.
2. Complex cation – Tris (ethylene diamine) nickel (II) thiosulphate.
3. Complex anion – Sodium Hexanitrocobaltate (III) The aim of this experiment is to
understand the preparation of a soluble cation (sodium)and a large anion
hexanitrocobaltate (III) and its use to precipitate a large cation (potassium)
4. Inorganic salt – Calcium or magnesium oxalate using PFHS technique
Unit III: Organic Chemistry
Qualitative Analysis of bi-functional organic compounds on the basis of
1. Prelimenary examination
2. Solubility profile
3. Detection of elements C, H, (O), N, S, X.
4. Detection of functional groups
5. Determination of physical constants (M.P/B.P)
Solid or liquid Compounds containing not more than two functional groups from among the
following classes may be given for analysisto be given: Carboxylic acids, phenol,
carbohydrates, aldehydes, ketones, ester, amides, nitro, anilides, amines, alkyl and aryl
halides.
Students are expected to write balanced chemical reactions wherever necessary. (Minimum 6
compounds to be analyzed)
Page 21
Reference Books for Practicals:
Unit I:
1. Khosla B.D., Garg V.C. and Gulati A., Senior Practical Physical Chemistry, R.
Chand and Co., New Delhi (2011).
2. Garland C. W., Nibler J.W. and Shoemaker D.P., Experiments in Physical Chemistry,
8th Ed., McGraw -Hill, New York (2003).
3. Halpern A.M. and McBane G.C., Experimental Physical Chemistry, 3rd Ed., W.H.
Freeman and Co., New York (2003).
4. Athawale V.D. and Mathur P., Experimental Physical Chemistry, New Age
International, New Delhi (2 001)
Unit II:
1. Practical Inorganic Chemistry by G. Marr and B. W. Rockett van Nostrand Reinhold
Company (1972)
Unit III:
1. Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009)
2. Ahluwalia, V.K. & Aggarwal, R. Comprehensive Pract ical Organic Chemistry:
Preparation and Quantitative Analysis, University Press (2000). Mann, F.G. &
Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009)
3. Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic
thChemistry, 5 Ed., Pearson (2012)
4. Vogel, A.I., Tatchell, A.R., Furnis, B.S., Hannaford, A.J. & Smith, P.W.G.,
Textbook of Practical Organic Chemistry, Prentice -Hall, 5th edition, 1996
Page 22
Reference Books:
Unit I:
1. Barrow, G.M. Physical Chemistry Tata McGraw‐Hill (2007).
2. Castellan, G.W. Physical Chemistry 4th Ed. Narosa (2004).
3. Kotz, J.C., Treichel, P.M. & Townsend, J.R. General Chemistry CengageLearning India
Pvt.Ltd., New Delhi (2009).
4. Mahan, B.H. University Chemistry 3rd Ed. Narosa (1998).
5. Petrucci, R.H. General Chemistry 5th Ed. Macmillan Publishing Co., NewYork (1985).
6. K.L.Kapoor A textbook of Physical Chemistry3rd Ed. vol.1,2Macmillan Publishing Co.,
NewDelhi(2001)
Unit II:
1. Practical Inorganic Chemistry by G. Marr and B. W. Rockett van Nostrand Reinhold
Compa ny (1972)
2. Inorganic Chemistry – Gary Wulfsberg, Viva Book, First Indian Edition 2002
3. Quantitative Analysis – R.A.Day, A.L. Underwood, sixth edition
4. Vogel’s Textbook of quantitative chemical analysis – J Mendham, R C Denny, J D Barnes, M
Thomas, B Sivasank ar
5. Bruce H. Mahan, University Chemistry, Narosa publishing house pg. 611 to 683.
6. R. Gopalan , Universities Press India Pvt.Ltd. Inorganic Chemistry for Undergraduates.
7. Chemistry of Transition Elements Pg.- 608 – 679 .
8. J. D. Lee, 4th Edn., Concise Inorganic Chemistry, ELBS, The group III elements Pg. 359 -
648.
9. D. F. Shriver and P. W. Atkins, Inorganic chemistry, 3rd edition, Oxford University Press
(1999) page 325 -446.
10. Ramesh Kapoor and R.S. Chopra, Inorganic Chemistry, R. Chand publishers, New Delhi.
11. CNR Rao edited, University General Chemistry, 513-578.
12. James E. Huheey, Inorganic Chemistry: Principles of Structure and Reactivity,
13. Emeleus and Anderson, Modern Aspects of Inorganic Chemistry, page no. 435-463.
14. Cotton and Wilkinson, Advanced Inorganic Chemistry , 3rd. Edition.
15. Gary Wulfsberg, Inorganic chemistry, Viva Books Pvt,. Ltd. (2002).
16. Puri, Sharma and Kalia, Milestone publishers, Principles of Inorganic Chemistry, page 416 -
628.
17. Bruce H. Mahan, University Chemistry, Narosa publishing house.
18. R. Gopalan , Universities Press India Pvt.Ltd. Inorganic Chemistry for Undergraduates.
19. J. D. Lee, 4th Edn., Concise Inorganic Chemistry, ELBS
20. D. F. Shriver and P. W. Atkins, Inorganic chemistry, 3rd edition, Oxford University Press
(1999)
21. Ramesh Kapoor and R.S. Chopra, Inorganic Chemistry, R. Chand publishers, New Delhi.
22. CNR Rao edited, University General Chemistry
23. James E. Huheey, Inorganic Chemistry: Principles of Structure and Reactivity,
Page 23
24. Emeleus and Anderson, Modern Aspects of Inorganic Chemistry
25. Cotton and Wilkinso n, Advanced Inorganic Chemistry, 3rd. Edition.
26. Gary Wulfsberg, Inorganic chemistry, Viva Books Pvt,. Ltd. (2002).
27. Puri, Sharma and Kalia, Milestone publishers, Principles of Inorganic Chemistry
Unit III:
1. Morrison, R. T. and Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.
(Pearson Education).2012
2. Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson
Education).
3. Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural
Produc ts), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education)
4. Mc Murry, J.E. Fundamentals of Organic Chemistry, 7th Ed. Cengage Learning India
Edition, 2013.
5. Clayden, J.; Greeves, N.; Warren, S.; Wothers, P.; Organic Chemistry, Oxford University
Press.
6. Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc.
7. Comprehensive Organic Chemistry - The synthesis and reactions of Organic
Compounds, Derek barton ,W. David Ollis.
8. Kalsi, P. S. Textbook of Organic Chemistry 1st Ed., New Age International (P) Ltd. Pub.
9. Eliel, E. L. and Wilen, S. H. Stereochemistry of Organic Compounds, Wiley: London,
1994.
10. Kalsi, P. S. Stereochemistry Conformation and Mechanism, New Age International, 2005
Page 24
Semester III
Paper III
Basics in analytical Chemistry
Theory: 45 Lectures
The Role of Analytical Chemistry in various fields including non-chemistry fields such as
Environmental Science, Pharmacy, Medicine, Life Sciences, Petrochemicals, Arts (like Painting)
Forensic sciences and so on can never be underesti mated. This course is expected to introduce the
learner to this interesting field of Analytical Chemistry.
It is expected to provide the learner an overview of this very important branch of chemistry. After
successful completion of this course the learner is expected to be familiar with the question of
what is analysis, why it is required and the methods, techniques, procedures and protocols that
may be used or required in the course of a given problem of analysis. The learner is also expected
to appreciate the role of an Analytical Chemist and a Chemical Analyst.
Correctness or acceptability of the results of a given analysis and how to deal with wrong or
erroneous results: when to reject them and when and how to retain them to be meaningful and/or
acceptab le are some other attributes expected as outcomes of learning this paper As such it is felt
that this paper will be a subject of choice and interest for learners preferring a specialization in
Chemistry as well as to those who may have interests in other s cience fields as Physics, Botany,
Zoology, Microbiology, Geochemistry and so on.
Goal:
To introduce the learner to an area of learning that is vital for the inherent nature of the subject
itself but also is important and irreplaceable irrespective of the long-term interest of specialization
or subject of interest of the learner.
Page 25
Unit I-Introduction to Analytical Chemistry and Statistical Treatment of analytical data -[15L]
Scope/Objectives:
Learners should be able to
1. Selecta method of analysis
2. Decide how to identify a sample and prepare it for analysis
3. Select a procedure for analysis
4. Identify sources of possible errors in the results obtained.
[Numerical problems wherever possible, expected]
1.1. Role of Analytical Chemistry [04 L]
1.1.1. Language of analytical chem istry: important terms and their significance in Analytical
Chemistry.
1.1.2. Purpose of Chemical Analysis; Analysis Based on
(i) the nature of information required:(Proximate, Partial, Trace, Complete Analysis) and
(ii) On the size of the sample used (Macro, semi-micro and microanalysis )
1.1.3. Classical and Non-Classical Methods of Analysis; their types and Importance .
1.2. Significance of Sampling in Analytical Chemistry [05 L]
1.2.1. Terms involved in Sampling
1.2.2. Purpose of Sampling
1.2.3. Difficulties encountered in sampling
1.2.4. Types of Sa mpling
i) Random Sampling
ii) Systematic Sampling
1.2.5. Theories of Sampling
1.3. Results of Analysis [06 L]
1.3.1. Errors in Analysis and their types
i) Determinate Errors
ii) Indeterminate Errors
1.3.2 Methods of minimizing Determinate errors in analysis
i) Calibration of apparatus
ii) Carrying out Control determination
iii) Carrying out Blank determination
1.3.3 Concept of Precision and Accuracy in Analysis and evaluation involved in the study of
Precision and accuracy
i) Mean, Median, Mode, Absolute deviation, Average deviation, Relative average
deviation, standard deviation, variance and coefficient of variation
ii) Absolute error and Relative error
[Numerical problems on precision and accuracy expected]
References:
1. Instrumental Analysis by Douglas A. Skoog , F. James Holler , Stanley R.Crouch
2. Instrumental methods of analysis by Willard, H.H. ; Merritt, L.L. Jr. ;Dean,J.A. ; Settle, 7th Edition
3. FundamentalofAnalyticalChemistryby DouglasA.Skoog ,West, F.JamesHoller ,S.R. Crouch
4. Modern Analytical Chemistry by David Harvey, McGraw -Hill Higher Education
Page 26
Unit II- Classical Methods of Analysis [15L]
Objectives:
The main objectives of this unit is to
Introduce classical methods of chemical analysis.
Appreciate the various terms and types of titrimetric analysis.
Ability to select proper titrimetric method
Appreciate the usefulness of the gravimetric method of analysis
Identify a suitable gravimetric method
Perform the requ ired calculations involved in the analysis by titrimetry as well
as gravimetry.
2. Classical Methods of Analysis. [15 L]
2.1. Titrimetric Methods [04 L]
2.1.1. Terms involved in Titrimetric methods of analysis. Comparing volumetry and
Titrimetry
2.1.2. The Conditions suitable for titrimetry
2.1.3. Types of titrimetry
i) Neutralisation (Acidimetry, alkalimetry)
ii) Redox (Iodometry, Iodimetry,)
iii) Precipitation
iv) Complexometric titrations
2.1.4. Tools of Titrimetry: Graduated glassware and Calibration
2.2. Standard solutions[02L]
2.1.1 Primary and Secondary standa rds in Titrimetry
2.1.2 Calculations based on preparation of primary and secondary standards
2.2 Neutralization Titration [03 L]
2.2.1 Concept of pH and its importance in Neutralization Titrations
2.2.2 Endpoint and Equivalence point of Neutralization titrations
2.2.3 Determination of End point by using Indicators causing colour change
2.2.4 Selection of indicators – Ostwald’s theory of indicators
2.3 Gravimetric analysis [06L]
2.3.1 Introduction and Principle of Gravimetric analysis
2.3.2 Types of Gravimetric Methods
i) Volatilisation gravimetry
ii) Precipitat ion gravimetry
2.3.3 Precipitation Gravimetry:
i) Steps involved in precipitation gravimetric analysis
ii) Factors affecting precipitation
iii) Concept of Nucleation (Homogenous and Heterogeneous) and crystal growth
iv) Impurities involved in precipitates
i) Simultaneous preci pitation
ii) Post precipitation
iii) Co-precipitation
2.3.4 Digestion and its importance
2.3.5 Filtration, Washing , Drying and Ignition of Precipitate .
2.3.6 Applications of Gravimetric Analysis:
i) Determination of sulfur from organic compounds;
ii) Estimation of Nickel in Cu -Ni alloy using dimethyl glyoxime
Page 27
References:
1) Skoog etal. “Fundamentals of Analytic al Chemistry " Cengage Learning, Eight Edition,
chapter13, 14 and 15
2) Day and Underwood, “Quantitative analysis" prentice hall 1991, chapter 3
3) S.M. Khopkar, “Basic Concepts of Analytical Chemistry”, IInd Edition New Age International
Publisher
4) Gary D. Christan, “Analytical Chemistry”, VIth Edition, Wiley Students Edition, Chapter No. 8, 9,
10
5) Fundamental of Analytical Chemistry by Douglas A. Skoog , West, F. James Holler , S. R. Crouch
6) Modern Analytical Chemistry, David Harvey (page numbers 232-265)
Unit III: Instrumental Methods -I [15 L]
Objectives:
On completing the learning of this unit the learner is expected to
Know the various instrumental methods of analysis
Advantages of using instruments to make measurements
The various observable properties of a given analyte and the stimulus best suited for
its analysis
Know about a generalized diagram of an analytical instrument
Select a suitable instrumental method for analysis
Appreciate the basic terms in spectrometry
Use the relationship betw een absorbance (and its variations) and concentration of the
analyte.
Chose a suitable method for photometric titrations.
3 Basic Concepts in Instrumental Methods [03 L]
3.1 Relation between the Analyte, Stimulus and measurement of change in the observable
property.
3.2 Block Diagram of an Analytical Instrument .
3.3 Types of Analytical Instrumental Methods based on
i. Optical interactions (eg. Spectrometry: UV-Visible, Polarimetry)
ii. Electrochemical interactions (eg. Potentiometry, Conductometry,)
iii. Thermal interactions (eg. Thermogravimetry)
3.4 Spec trometry [12 L]
3.4.1 Interaction of electromagnetic radiation with matter: Absorption and Emission
spectroscopy
3.4.2 Basic Terms: Radiant Power, Absorbance, Transmittance, Monochromatic light,
Polychromatic light, Wavelength of maximum absorba nce, Absorptivity and Molar
Absorbtivity
3.4.3 Statement and derivation of Beer’s Law and Lambert’s Law, Combined Mathematical
Expression of Beer Lambert’s Law,
3.4.4 Validity and Deviations from Beer -Lambert’s Law (Numerical problems based on Beer -
Lambert’s Law)
3.4.5 Block Diagrams for Single beam and double beam Colorimeter (Principle, Construction and
working (Det ails of Components expected, i.e. source, Sample holder, Filter, Detectors)
3.4.6 Block Diagrams for Single beam and double beam Spectrophotometer (Principle,
Constr uction and working (Details of Components expected i.e, source, Sample holder,
Monochromator, Detectors)
Page 28
References:
1. Instrumental Methods of Chemic al Analysis by Gurdeep R. Chatwal, Sh m K. Anand pp2.107 -2.148
2. Principles of Instrumental Analysis by Skoog , Holler, Nieman, 5th Edition pp143 -172.
3. Instrumental Methods of Analysis by Willard, Merritt, Dean, Settle 7th Edition pp 118 -
181.
Semester III Chemistry
Practicals: Paper III
Basics in Analytical Chemistry
1. Tools of Analytical Chemistry -I:
a) Analytical gl ass wares like burettes, pipettes, Standard flasks, Separating funnels.
b) Weighing tools such as two pan balance and mono pan balance, digital balances:
c) Incineration devices: Burners, Electrical Incinerators, Muffle Furnace,
d) Drying Devices: Hot Air Oven, microwave oven , Desiccators, Vacuum desiccators
e) Monochromators, Filters, Sample holders, Prisms, Diffraction Gratings,
Photoemissive cells, Photomultiplier tubes
(The learner should draw diagrams and write -ups providing uses, care and maintenance of the
items mentioned in (a)and principle, construction and uses of items(b)to (e)in his journal.
2. Gravimetric estimation of Nickel (II) as Ni -DMG and calculation of % error.(The learner is
expected to know the role of the various reagents/chemicals used in the estima tion, the various
steps involved. They should write the complete and Balanced chemical reaction for t he formation
of the Ni(DMG) 2 complex.
3. Colorimetric Determination of Copper Ions in a given Solution by using calibration curve method
and calculation of % error.
(The learner is expected to learn the relation between concentration and Absorbance, to draw a
calibration curve, use the slope of the calibration curve and compare it with the calculated slope.
They are also expected to state the error estimate of their results).
4. Determination of buffer capacity of acid buffer and basic buffer.
(The learner is expected to learn the use pH meter, standardization of pH meter, use of Henderson’s
equation a nd calculation of buffer capacity)
5. Estimation of Aspirin
6. Gravi metric estimation of barium ions using K 2CrO 4 as precipitant. Calculation of % error.
(The learner is expected to learn the skills of using the counterpoise technique used in this
gravimetric estimation; Using counterpoise method whatman No.42 for filtrat ion. In such a case no
incineration or use of silica crucible is required. They are also expected to state the error estimate of
their results)
Page 29
Semester IV
Paper III : Basics in Analytical Chemistry -II
Theory:45 Lectures
Unit–I –Methods of separation [ 15L]
Objectives
The learner is expected to understand
The importance of separation in sample treatment
Various methods of separations
How to select a method of separation of an analyte from the matrix
How a solute gets distributed between two immiscible phases
Principle of solvent extraction and various terms involved therein
Effect of various parameters on solvent extraction of a solute
Classification of Chromatographic methods
Paper and thin layer chromatography and using them in practice.
1. Separation Techniques in Analytical Chemistry [02L]
1.1. An Introduction to Analytical Separations and its importance in analysis.
1.2. Estimation of an analyte without a ffecting separation.
1.3. Types of separation methods
1.3.1. Based on Solubilities (Precipitation, Filtration Crystall isation)
1.3.2. Based on Gravity -Centrifugation
1.3.3. Based on volatility -Distillation;
1.3.4. Based on Electrical effects -Electrophoresis
1.3.5. Based on retention capacity of a Stationary Phase -Chromatography;
1.3.6. Based on distribution in two immiscible phases -Solvent Extraction;
1.3.7. Based on capacity to exchange with a resin -Ion Exchange;
1.4. Study of types of separation methods
1.4.1 Electrophoresis: [02 L]
Principles, Basic Instrumentation, Working and Application in separ ation of
biomolecules like enzymes and DNA.
1.4.2 Solvent extraction [06L]
i) Introduction, Nernst distribution Law, Distribution Ratio, Partition Coefficient and
Separation factor.
ii) Conditions of extraction: Equilibration time, Solvent volumes, temperature, pH.
iii) Single-step and multistep extraction, Percentage extraction for single step and
multistep extraction.
iv) Batch and continuous extraction
1.5 Chromatography: [05L]
1.5.1 Introduction to Chromatography
1.5.2 Classification of chromatographic methods based on stationary and mobil e phase
1.5.3 Paper Chromatography
i) Principle
ii) Technique
iii) Applications in separation of cations.
1.5.4 Thin layer Chromatography
i) Principle
ii) Technique
iii) Applications with special reference to
a) Determination of the purity of a given solute
b) Study of the progress of a given rea ction.
Page 30
References:
1. D.A. Skoog, D.M. West, F.J. Holler and CX.R. Crouch – Fundamentals of
Analytical Chemistry , 8th edition
2. G. H. Morrison and H. Freiser, Solvent extraction in analytical chemistry
3. P.G. Swell and B. Clarke, Chromatographic separations, Anal ytical chemistry by open
Learning, John Wiley and sons, 1987
4. Modern Analytical Chemistry, David Harvey (page numbers 596-606)
5. Modern Analytical Chemistry, David Harvey (page numbers 215-217)
Unit–II-Instrumental Methods -II [15 L]
Objectives
On completing this unit, the learner is
Expected to appreciate the nature of interaction between applied electrical potential and
the concentration of the analyte.
The nature of chemical reactions that influence potential of a given cell.
Familiar with the various types of electrodes or half cells.
Appreciate the nature, need and importance of pH
Expected to know the applications of the various instrumental methods dealt with in this
unit.
2. Instruments based on the electrochemical properties of the analytes
2.1. Potentiometry: [05 L]
2.1.1. Principle.
2.1.2. Role of Reference and indicator electrodes
2.1.3. Applications in Neutralization reactions with reference to the titration of Strong
acid against Strong Base (using quinhydrone electrode)
2.1.4. Graphical methods for detection of endpoints
i) Graph of EMF against Volume of titrant added
ii) First derivative graph
2.2. pH metry: [04 L]
2.2.1. Principle
2.2.2. Construction , working and maintenance of Combined Glass electrode
2.2.3. Application
i) In Titrimetry (Strong acid-Strong Base)
ii) Biological and Environmental analysis.
2.3. Condu ctometry: [06 L]
2.3.1. Principle
2.3.2. Conductivity cell: Construction
2.3.3. Applications in Neutralization Titrimetry with respect to
i. Strong Acid -Strong Base
ii. Strong Acid -Weak Base
iii. Strong Base -weak Acid
iv. Weak Acid - Weak Base .
2.3.4. Advantages and limitations of conductometri c titrations.
References:
1) Principles of Instrumental Analysis , D. A. Skoog, 3rd edition, Saunders College publishing.
Chapters:20, 23Page Nos: 600 -605, 631, 704 - 711.
2) Vogel’s Textbook of quantitative inorganic analysis, 4thedition, ELBS / Longman. Chapte rs: XIV,
XV Page nos:566 - 601, 615 – 625.
3) Instrumental method of analysis , B.K. Sharma, Goel publishing house. Miscellaneous methods:
Chapters:1,3,4 Page Nos: 1 -14, 21 - 57.
Page 31
Unit III-Statistical Treatment of analytical data—II [15L]
Objectives: On completi ng this unit the learner is expected to understand
i) The use of statistical methods in chemical analysis.
ii) Therandomnessofsucherrorsanditsdistributionaroundacorrectoracceptableresult
iii) Computation of Confidence limits and confidence interval
iv) Test for rejection of doubtful result
v) Method to draw best fitting straight line
3.1. Distribution of random errors: [03L]
3.1.1. Gaussian distribution curve.
3.1.2. Equation and salient features of Gaussian distribution curve
3.2. Concept of Confidence limits and confidence interval and its computa tion using [04 L]
(i) Population standard deviation
(ii) Student’s test
(iii) Range
3.3. Criteria for rejection of doubtful result [03 L]
(i) 2.5 d rule
(ii) 4.0 d rule
(iii) Q test
3.4. Test of Significance [03 L]
(i) Null hypothesis
(ii) F-test (variance ratio test)
3.5. Graphical representation of data and obtaining best fitting straight line [02L]
(i) For line passing through origin
(ii) For line not passing through origin
Note: Numerical problems on 3.2 to 3.5 are expected
References:
1. Modern Analytical Chemistry, David Harvey (page numbers 53 -84)
2. Fundamentals of analytical chemistry –Skoog and West
Page 32
Semester IV
Chemistry Practicals:
Paper III Elective (Basics in Analytical Chemistry)
1. Tools of Analytical Chemistry -II
a. Filtration Flasks, Funnels, Separating Funnels, Distillation appara tus, Vacuum
Distillation assembly, Centrifuge machine, Electrophoresis apparatus.
b. Development chamber for chromatography
c. Electrodes like Reference Electrodes and Indicator Electrodes (with respect to care
and maintenance.)
d. Conductivity cell (with respect t o care and maintenance.)
e. Combined Glass electrode (with respect to care and maintenance.)
f. Types of Salt Bridges and preparation of anyone or use of a salt bridge, its effect
on the potential of a given electrode/cell
(The learner should draw diagrams and write-ups providing uses of the items mentioned in (a and
b) and Principle, Construction care and Uses of items (c) to (f) in his journal.)
2. Paper chromatography: Separation of cations like Fe (III), Ni (II) and Cu (II) in a sample.
3. Separation of a solute be tween two immiscible solvents to determine the distribution
ratio and/or extraction efficiency. (Solutes could be as their aqueous solutions and the
organic solvent ethyl acetate) Suggested solute for the distribution study: Fe (III) in
aqueous solutions. (The learner is expected to learn the technique of solvent extraction
by using a separating funnel, method to estimate the concentrations of the solute
distributed in the two immiscible phases, determination of the extraction efficiency)
4. Estimation of conc entration of Iron from a given sample calorimetrically by using
1,10 phenanthroline.(The learner is expected to learn the handling of the colorimeter ).
5. Estimation of Fe (II) in the given solution by titrating against K 2Cr2O7
potentiometrically and calcul ation of % error. (The learner is expected to learn the
handling of the potentiometer, use of Platinum electrode and reference electrode like
SCE. They will learn to determine endpoint by plotting a graph. They are also expected
to state the error estimate of their results).
6. Gravimetric estimation of Sulfate as BaSO 4 and calculation of % error. (The learner is
expected to write a balanced chemical reaction, need for digestion of the precipitate
and the skill required to carry out the incineration and to est imate the% error.)
(The learner is expected to write a balanced chemical reaction, need for digestion of the
precipitate and the skill required to carry out the incineration and to estimate the %
error.)
REFERENCES:
For paper III
1. D.A. Skoog, D.M. West, F.J. Holler, and S.R. Crouch, Analytical Chemistry: An
Introduction,7th ed., Chapter 15, pp. 345 -381.
2. A.I. Vogel.“Text book of Quantitative Inorganic Analysis” , Longman, London (1961).
3. R.V. Dilts.“Analytical Chemistry. Methods of Separation” , van Nostran d, N.Y.(1974).
4. Some Experiments for B. Tech in Chemistry & Chemical Technology compiled by Prof. J.B.
BARUAH, Mrs. Abhilasha Mohan Baruah and Mr. Parikshit Gogoi .
Prof. Shivram S. Garje,
Dean ,
Faculty of Science and Technology
Page 33